In a cell a copper electrode was used as a cathode. What is the electrode potential (in V) of the copper electrode dipped in $0.1 \mathrm{M} \mathrm{Cu}^{2+}$ solution at 298 K ?

$$ \left(E_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\ominus}=0.34 \mathrm{~V} ; \frac{2.303 R T}{F}=0.06 \mathrm{~V}\right) $$

Observe the following statements about dry cell

I. It is a primary battery.

II. Zinc vessel acts as cathode.

III. A paste of moist $\mathrm{NH}_4 \mathrm{Cl}, \mathrm{MnO}_2$ and $\mathrm{ZnCl}_2$, is present between two electrodes

IV. The potential of this cell is 1.5 V .

The correct statements are

$$ \text { Match the following } $$

$$ \begin{array}{llll} \hline & \begin{array}{l} \text { List-I (Symbol of } \\ \text { electrical property) } \end{array} & & \text { List-I (Units) } \\ \hline \text { (A) } & \Lambda_{\mathrm{m}} & \text { (I) } & \mathrm{Scm}^{-1} \\ \hline \text { (B) } & \mathrm{G} & \text { (II) } & \mathrm{m}^{-1} \\ \hline \text { (C) } & \mathrm{K} & \text { (III) } & \mathrm{Scm}^2 \mathrm{~mol}^{-1} \\ \hline \text { (D) } & \mathrm{G}^* & \text { (IV) } & \mathrm{S} \\ \hline \end{array} $$

The correct answer is

Consider the following cell reaction

$$ 2 \mathrm{Fe}^{3+}(a q)+2 \mathrm{I}^{-}(a q) \rightleftharpoons 2 \mathrm{Fe}^{2+}(a q)+\mathrm{I}_2(s) $$

At 298 K , the cell emf is 0.237 V . The equilibrium constant for the reaction is $10^x$. The value of $x$ is $\left(F=96500 \mathrm{C} \mathrm{mol}^{-1} ; R=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$.